Chemistry Paper 2 Questions and Answers - Kassu Jet Joint Exams 2020/2021

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Instructions to Candidates

  • Answer ALL the questions in the spaces provided.
  • Mathematical tables and silent electronic calculators may be used.
  • All working MUST be clearly shown where necessary.


    1. Consider the following reaction:
      A2(g) + B2(g)  ⇌ 2AB(g), ΔH = +75 kJ
      Sketch an energy level diagram showing the relative activation energies for the catalysed and uncatalysed reactions using the axes below. (2mks)
    2. Given that; ΔHf (Al2O3) = – 1590 kJmol-1
      ΔHf (Cr2O3) = -1134 kJmol-1
      Calculate the heat of reaction for; 2Al(s) + Cr2O3(s) → Al2O3(2mks)
    3. The following data was obtained during an experiment
      Mass of ethanol burnt = 0.2g
      Mass of water in the calorimeter = 200g
      Specific heat capacity of water = 4.2 jg-1k-1
      Initial temperature of water = 23.5 0C
      Final temperature of water = 28.0 0C
      1. How was the mass of ethanol that burnt determined? (1mk)
      2. How much heat was required to raise the temperature of water from 23.5 0C to 28.00C? (2mks)
      3. Two assumptions were made in calculating the enthalpy of combustion for ethanol. State them. (1mk)
      4. Determine the molar enthalpy of combustion of ethanol.(C= 12,H=1, O=16) (2mks)
      5. Write a thermochemical equation for the combustion of ethanol given the accurate value for enthalpy of combustion is – 1368 kJmol-1. (1mk)
  2. Two half cells were connected as shown to form a voltaic cell. The reduction potentials are given.
    voltaic cell q2
    Pb2+(aq) + 2e- → Pb(s) EӨ = – 0.13V
    Fe2+(aq) + 2e- → Fe(s) EӨ = – 0.44V
    1. Calculate the e.m.f of the cell. (1mk)
    2. Sodium chloride is used as the salt bridge. State the two functions of the salt bridge. (2mks)
    3. Show the direction of the electron flow in the external circuit. (1mk)
    4. The e.m.f of the cell will reduce with time. Give a reason for this. (1mk)
    5. During electrolysis of water acidified with Sulphuric acid, two gases were produced at the electrodes:
      1. State which ions are preferentially discharged at the electrodes. Explain with aid of half ionic equations.
        Anode. (2mks)
        Cathode. (2mks)
      2. Calculate the volume of the gases at s.t.p produced when a current of 0.025A is passed for 4 hours. (1 Faraday=96500C) (3mks)
    1. The fermentation of glucose is catalysed by enzymes from yeast. Yeast is added to aqueous glucose, the solution starts to bubble and becomes cloudy as more yeast cells are formed.
      C6H12O6(aq) → 2C2H5OH(aq) + 2CO2(g)
      The reaction is exothermic. Eventually the fermentation stops when the concentration of ethanol is about 12%.
      1. On a large scale, the reaction mixture is cooled. Suggest a reason why this is necessary. (1mk)
      2. Why does the fermentation stop? Suggest one reasons. (1mk)
      3. What technique is used to concentrate the aqueous ethanol? (1mk)
    2. A compound X contains carbon, hydrogen and oxygen only. X contains 54.54% of carbon by mass, 9.09% of hydrogen by mass and 36.37% of oxygen by mass. (C=12, O=16, H=1)
      1. Determine the empirical formula of compound X. (2mks)
      2. Compound X has a relative molecular mass of 88. Draw the structural formula of compound X. (2mks)
    3. The table below gives formulae of three organic compounds A, B and C
       Compound  Formulae
       A  C2H4O2
       B  C2H6O
       C  C2H6

      Giving a reason in each case, select the letter(s) which represent a compound that
      1. Decolourises acidified potassium manganate (VII). (1mk)
      2. Gives effervescence with sodium hydrogen carbonate. (1mk)
      3. Undergoes substitution reaction with chlorine gas. (1mk)
    4. The following is a small reaction of polystyrene polymer. Study it and answer the questions that follow.
      polystyrene polymer p2
      1. Draw the structure of the monomer unit of polystyrene. (1mk)
      2. Calculate the number of monomers used to form the polystyrene of relative molecular mass of 18096. ( H = 1, C = 12 ) (1mk)
  4. An experiment was carried out using magnesium ribbon and dilute hydrochloric acid of different concentrations. The time needed to produce 50cm3 of the gas for every experiment was recorded in a table.
     Concentration of HCL (moles per litre)  2.0  1.75  1.50  1.25  1.00  0.75  0.50  0.25
     Time (seconds)  8.8  10.0  11.7  14.0  17.5  18.7  35.0  70.0
     1/time (sec-1)                
    1. Complete the table above for 1/time. (4mks)
    2. Plot a graph of rate i.e 1/time against concentration. (3mks)
    3. From your graph determine the concentration needed to produce 50cm3 of hydrogen gas when time is 15.0 seconds (1mks)
    4. From your graph state the relationship between the rate of reaction and concentration. Give a reason. (1mk)
    5. A state of equilibrium between dichromate (VI) and chromate ions is established as shown below
      Cr2O72-(aq) + 2OH-(aq) ⇌  2CrO42-(aq) + H2O(l)
      Orange                            Yellow
      1. What is meant by dynamic equilibrium? (1mk)
      2. State and explain observation made, when a few pellets of Hydrochloric acid are added to equilibrium mixture ( 2mks)
    1. The table below shows properties of some elements represented by symbols W,X,Y and Z. Study the information in the table and answer the questions that follows
       Element  No. of Protons  Atomic Radius (nm)  Boiling point oC
       W  2  0.93  -269
       X  10  1.31  -246
       Y  18  1.54  -186
       Z  36  1.89  -152
      1. Write down the electron arrangement for elements W and X (1mk)
      2. In which group of the periodic table are the elements in the table above? Give the name of the group (2mks)
      3. Explain why the atomic radius of W is smaller than that of X (1mk)
      4. state one use of element X (1mk)
    2. The section below represents part of the periodic table. Study it and answer the questions that follow. The letters are not the actual symbol of the elements.
      periodic table q5II
      1. Select the least reactive non-metal. (1mk)
      2. Which of the elements has the greatest tendency of forming covalent compounds in nature? Explain your choice. (1mk)
      3. Explain why the atomic radius of T is smaller than that of M. (2mks)
      4. Compare the electrical conductivity of element X and B. (2mks)
  6. Extraction of iron involves two main processes, smelting and refining. Below is the blast furnace which is used to smelt iron from its ore.
    extraction of iron q6
      1. The chief ore is Haematite. Name one other ore used in extraction of iron (1 mark)
      2. What is the role of the hot air blast in the process? (2mks)
    2. Write equations for the reactions that take place at the region marked A, B and C. (3mks)
      C ………………………………………………………………………
    3. What is the purpose of limestone in the extraction process? (1mk)
    4. Write equations to show how impurities are removed from the ore. (2mks)
    5. State one environmental effect of the process. (1mk)
    1. Read the following passage and answer the questions.
      A salt K was heated with slaked lime (calcium hydroxide). A colourless gas L with a characteristic smell and turns red litmus paper blue was evolved. A large quantity of this gas was passed through an inverted filter funnel into Copper(II)sulphate solution, and a deep blue solution M was obtained.
      1. Identify gas L (1mk)
      2. What is K most likely to be? (1mk)
      3. Write an equation for the reaction between K and slaked lime (1mk)
      4. Write an ionic equation for the reaction with copper(II) sulphate forming the deep blue solution (1mk)
    2. Study the flow chart below and answer questions that follow:
      1. State one source of gas B (1mk)
      2. Name the catalysts used in; (1mk)
        1. Step I
        2. Step III
      3. Write chemical equations for reactions in; (3mks)
        1. Step I
        2. Step II
        3. Step V
      4.  Identify any other gas that can be used instead of Ammonia in step II (1mk)
      5. State one use of gas Q (1mk)

Marking Scheme

      1. By subtracting the mass of the burner and ethanol before igniting and the mass of the burner and ethanol after the burning
      2. Heat produced ΔH = mass of water (m) × specific heat capacity (c) × ΔT
        = 200 × 4.2 × 4.5 = 3780 joules = 3.78kJ
      3. - No heat loss to the environent
        - The calorimeter did not absorb any heat
      4. Moles of ethanol used = 0.2/46
        = 0.0043 moles → 3.78 kJ
           1 Mole           →  ?
        = 3.78 × 1/0.0043
        = -879.069 kJ/mol
      5. C2H5OH +3O2(g) →2CO2(g)+3H20(l)     ΔH = – 1368 kJmol-1.
    1. ERedox = ERed − EOx = −0.13 −− 0.44
    2. - complete the circuit
      - maintain balance of charges/ions on both half cells
      1. Anode.                                                                                                           (2mks)
        OH-(aq) from water (H2O)
        4OH-(aq)   →  2H2O(l) + O2(g) +4e-
        OH- ions selectively discharged instead of SO42- ions at the anode

        Cathode.                                                                                                         (2mks)
        H+(aq) from either sulphuric(VI) acid (H2SO4) or water (H2O)
        H+(aq) + 4e-  →  2H2(g)
      2. Quantity of electricity (in Coulombs) = Current (I) x time (t)
        Substituting/converting time to second = 0.025 x (4 x 60 x 60)
        = 360 C
        Anode; 4 moles of electrons = 4 Faradays
        96500 x 4 C → 22400cm3
        360C →
        360 x 22400
        96500 x 4
        Cathode; ratio 1;2
        20.89 x 2 = 41.78cm3

      1. kill  yeast or denature enzymes (due to increase in temperature)
      2. - All glucose used up
        - yeast killed or denatured or damaged by ethanol/alcohol
      3. Fractional distillation
         Element  C  H  O
         Mass  54.54  9.09  36.37
         R.A.M  12  1  16
         Moles  54.54/12  9.09/1  36.37/16
         Mole Ratio  4.545/2.273
        = 2
        = 3.99 ≈ 4
        = 1
      2. (C2H4O)n=88 H
        (C2H4O)2= C4H8O2 

      1. B - It's an alkanol hence oxidized to alkanoic acid
      2. A Reacts to produce CO2
      3. C - its saturated
        styrene monomer
      2. 18096/104
        = 174 monomers
       Concentration of HCl (moles per litre)  2.0  1.75  1.50  1.25  1.00  0.75  0.50  0.25
       Time (seconds)  8.8  10.0  11.7  14.0  17.5  18.7  35.0  70.0
       1/time (sec-1)  0.1140  0.1000  0.0854  0.0714  0.0571 0.0534  0.0286  0.0143
       1/t × 10-2  11.4  10.0  8.54  7.14  5.71  5.34  2.86  1.43
      graph of inverse of time against concentration min
    3. T=15
      1/15 = 1.1625
      = 1.1625
    4. Rate of reaction increases with increase in concentration
      1. - A reaction in which the rate of forward reaction is equal to the rate of backward reaction
        - Balance of the rate of formation of products and reactants
      2. - Solution mixture makes it to be more Orange in colour.
        - Hydrochloric acid/H+(aq) is added to the equilibrium mixture a stress is created on the reactant side on the OH(aq). H+ ions react with OH(aq) to form water.
        - The equilibrium shift backward to the left to add/replace the 2OH(aq) that have reacted with the H+(aq) ions .More Cr2O7 (aq) ions formed in the
      1. W = 2
        X  = 2:8
      2. Group VII
      3. X has more/2 energy levels than W (1 energy levels).
      4. - Use in making neon advertising coloured signs
        - Used to make high voltage indicators
        - Neon and helium are used in making gas lasers
        - Liquid helium is an economical refrigerant
      1. M
      2. Q or H, group IV ,have a valency of 4 hence can share its 4 pairs of electrons
      3. T has more protons(18) hence higher nuclear charge than M (17 protons) attracting outermost electrons closer to the nucleaus reducing the atomic radius
      4. B has higher conductivity,it has 3 delocalised electrons X has 1 delocalised electrons
      1. Magnetite/Siderite
      2. Carbon(II)oxide
      3. -Reacts with coke/charcoal/carbon to form carbon(IV)oxide gas
        -raises the temperature at the bottom of the furnace to about 2000K(1650oC).
    2. A  - C(s)+O2(g) → CO2(g)
      B  - Fe2O3(s)+3CO(g) →2Fe(s)+CO2(g)
            Fe3O4(s)+4CO(g) →3Fe(s)+4CO2(g)
      C - CaCO3(s) →CaO(s) + CO2(g)
    3. decomposes to quicklime /calcium oxide which reacts to remove impurities and produce more carbon(IV)oxide gas.
    4. CaO(s) + SiO2(s) → CaSiO3(l)
      CaO(s) + Al2O3(s) →CaAl2O4(l)
      • Carbon(IV)oxide(CO2) gas is a green house gas that causes/increases global warming if allowed to escape/leak from the furnace.
      • Carbon(II)oxide(CO)gas is a highly poisonous/toxic odourless gas that can kill on leakage. It is preferentially absorbed by the haemoglobin in mammals instead of Oxygen to form a stable compound that reduce free hemoglobin in the blood.
      • Haematite (Fe2O3), Magnetite(Fe3O4) and Siderite (FeCO3) are extracted through quarrying /open cast mining that cause soil / environmental degradation .
      1. Ammonia
      2. Ammonium chloride
      3. Ca(OH)2(s) + NH4Cl(s) → CaCl2(aq) + H2O(l) + 2NH3(g)
      4. Cu(OH)2(s) + 4NH3(aq) → [Cu(NH3)4]+ (aq) + 2OH(aq)
      1. Fractional distillation of liquid air

        1. Finely divided iron
        2. Platinum or platinum rhodium
        1.                        Fe
          N2(g)+3H2(g) → 2NH3(g)
        2. 2NH3(g)+3CuO(s) → N2(g) + 3H2O(l) + 3Cu(s)
        3. NH3(aq) + HNO3(aq) → NH4NO3(aq)
      4. Hydrogen/Carbon(II)oxide
      5. - Used in the Haber process in the manufacture of ammonia.
        - Due to its inert nature, it is mixed with argon to fill electric bulbs (to avoid soot formation).
        - In liquid state it is used as an inert refrigerant e.g. storage of semen for artificial insemination.
        - Due to its inert nature, it is used in food preservation particularly for canned products i.e. it prevents combination of oxygen and oil which tends to enhance rusting.
        - It is used in oil field operation called enhanced oil recovery where it helps to force oil from subterranean deposits.

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